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  2. Dipolar compound - Wikipedia

    en.wikipedia.org/wiki/Dipolar_compound

    In organic chemistry, a dipolar compound or simply dipole is an electrically neutral molecule carrying a positive and a negative charge in at least one canonical description. In most dipolar compounds the charges are delocalized . [ 1 ]

  3. Dipole - Wikipedia

    en.wikipedia.org/wiki/Dipole

    A simple example of this system is a pair of charges of equal magnitude but opposite sign separated by some typically small distance. (A permanent electric dipole is called an electret.) A magnetic dipole is the closed circulation of an electric current system. A simple example is a single loop of wire with constant current through it.

  4. Chemical polarity - Wikipedia

    en.wikipedia.org/wiki/Chemical_polarity

    For example, the water molecule (H 2 O) contains two polar O−H bonds in a bent (nonlinear) geometry. The bond dipole moments do not cancel, so that the molecule forms a molecular dipole with its negative pole at the oxygen and its positive pole midway between the two hydrogen atoms. In the figure each bond joins the central O atom with a ...

  5. Intermolecular force - Wikipedia

    en.wikipedia.org/wiki/Intermolecular_force

    An example of a dipoledipole interaction can be seen in hydrogen chloride (HCl): the positive end of a polar molecule will attract the negative end of the other molecule and influence its position. Polar molecules have a net attraction between them. Examples of polar molecules include hydrogen chloride (HCl) and chloroform (CHCl 3).

  6. Hyperpolarizability - Wikipedia

    en.wikipedia.org/wiki/Hyperpolarizability

    The linear electric polarizability in isotropic media is defined as the ratio of the induced dipole moment of an atom to the electric field that produces this dipole moment. [ 5 ] Therefore, the dipole moment is:

  7. Polarizability - Wikipedia

    en.wikipedia.org/wiki/Polarizability

    The polarizability of an atom or molecule is defined as the ratio of its induced dipole moment to the local electric field; in a crystalline solid, one considers the dipole moment per unit cell. [1] Note that the local electric field seen by a molecule is generally different from the macroscopic electric field that would be measured externally.

  8. Cation–π interaction - Wikipedia

    en.wikipedia.org/wiki/Cation–π_interaction

    For example, if induced dipole was a controlling effect, aliphatic compounds such as cyclohexane should be good cation–π partners (but are not). [4] The cation–π interaction is noncovalent and is therefore fundamentally different than bonding between transition metals and π systems.

  9. Non-covalent interaction - Wikipedia

    en.wikipedia.org/wiki/Non-covalent_interaction

    A hydrogen bond (H-bond), is a specific type of interaction that involves dipoledipole attraction between a partially positive hydrogen atom and a highly electronegative, partially negative oxygen, nitrogen, sulfur, or fluorine atom (not covalently bound to said hydrogen atom). It is not a covalent bond, but instead is classified as a strong ...